The volume of $0.1 \ M$ oxalic acid that can be completely oxidized by $20 \ mL$ of $0.025 \ M$ $KMnO_4$ solution is (in $mL$)

The normality of $2 \ M$ sulphuric acid is: (in $N$)

Normality of $2 \, M$ sulphuric acid is

$C_2H_4$ can react with $H_2$ in the presence of a catalyst to form $C_2H_6$ as per the following reaction: $C_2H_{4(g)} + H_{2(g)} \xrightarrow{\text{Catalyst}} C_2H_{6(g)}$. The amount of $C_2H_4$ in grams required to produce $50 \ g$ of $C_2H_6$ is: (in $g$)

The density (in $g \; mL^{-1}$) of a $3.60 \; M$ sulphuric acid solution that is $29 \%$ $H_2SO_4$ (molar mass $= 98 \; g \; mol^{-1}$) by mass will be

$X$ litres of carbon monoxide is present at $STP$. It is completely oxidized to $CO_2$. The volume of $CO_2$ formed is $11.207$ litres. What is the value of $X$ in litres?